Five moles of ${\mathrm{NH}}_3\left(\mathrm{g}\right)$ in a sealed vessel, dissociates as $2{\mathrm{NH}}_3\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)$ Calculate the equilibrium constant, if at equilibrium, one mole of ${\mathrm{N}}_2$ is found to be present.

$4{\mathrm{NH}}_{3\left(\mathrm{g}\right)}+5{\mathrm{O}}_{2\left(\mathrm{g}\right)}\rightleftharpoons 4{\mathrm{NO}}_{\left(\mathrm{g}\right)}+6{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{g}\right)}$

If two moles, each of ${\mathrm{NH}}_3$ and ${\mathrm{O}}_2$ are allowed to react, and the equilibrium is attained after $50\%$ of the ${\mathrm{O}}_2$ has reacted, what is the value of the equilibrium constant $\left({\mathrm{K}}_{\mathrm{C}}\right)$?

For the following reaction, ${\mathrm{K}}_{\mathrm{c}}=2\times {10}^{-3}$

$2 \mathrm{A}\rightleftharpoons \mathrm{B}+\mathrm{C}$

Identify the correct statement for the reaction when $\left[\mathrm{A}\right]=\left[\mathrm{B}\right]=\left[\mathrm{C}\right]=3\times {10}^{-4} \mathrm{M}$